•To calculate the mass of oxygen that will be used up for combustion of 5 grams of hydrogen gas (H2), we need to apply the law of constant proportions.
•The law of constant proportions states that in a chemical substance, the elements are always present in definite proportions by mass 1.
•The balanced chemical equation for the combustion of hydrogen gas is:
2H2 + O2 → 2H2O
•According to the law of constant proportions, the ratio of the masses of hydrogen and oxygen in water is always 2:16 or 1:8 .
Therefore, 1 gram of hydrogen requires 8 grams of oxygen for complete combustion.
•Using the above information, we can calculate the mass of oxygen required for the combustion of 5 grams of hydrogen as follows:
Mass of oxygen required = (Mass of hydrogen * 8) / 1
= (5 g * 8) / 1
= 40 g
Therefore, the mass of oxygen that will be used up for the combustion of 5 grams of hydrogen gas is 40 grams.
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•To calculate the mass of oxygen that will be used up for combustion of 5 grams of hydrogen gas (H2), we need to apply the law of constant proportions.
•The law of constant proportions states that in a chemical substance, the elements are always present in definite proportions by mass 1.
•The balanced chemical equation for the combustion of hydrogen gas is:
2H2 + O2 → 2H2O
•According to the law of constant proportions, the ratio of the masses of hydrogen and oxygen in water is always 2:16 or 1:8 .
Therefore, 1 gram of hydrogen requires 8 grams of oxygen for complete combustion.
•Using the above information, we can calculate the mass of oxygen required for the combustion of 5 grams of hydrogen as follows:
Mass of oxygen required = (Mass of hydrogen * 8) / 1
= (5 g * 8) / 1
= 40 g
Therefore, the mass of oxygen that will be used up for the combustion of 5 grams of hydrogen gas is 40 grams.
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